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2 litres of 9.8% (w/w) H2SO4 solution with density 1.5 g/mL is mixed with 3 litres of 1 M KOH solution. Find the concentration of H+ (if solution is acidic) or OH- (if solution is basic) in the final solution.

1. 0 M
2. 3/10 M
3. 3/5 M
4. 2/5 M

Correct answer: 3/5 M

Solution

Mass of 2 L solution = 3000 g. Mass of H2SO4 = 0.098 * 3000 = 294 g. Moles of H2SO4 = 294/98 = 3 mol. H+ equivalents = 6 (diprotic acid). KOH moles = 1 * 3 = 3 mol = 3 equivalents OH-. Excess H+ = 6 - 3 = 3 equivalents. Total volume = 5 L. [H+] = 3/5 M.

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